This MCAT General Chemistry Review Summary Page is by no means an exhaustive review of MCAT General Chemistry. Our summary is only meant to highlight key points that are most helpful for the MCAT. For a list of topics for the MCAT: MCAT General Chemistry Topics List. You can also access practice questions in our Free MCAT Practice Test, or our many fulllength MCAT Practice Tests.
For MCAT General Chemistry, it helps to understand vocabulary, definitions and equations. In some respects, this General Chemistry cheat sheet will minimize your need to memorize information and maximize your General Chemistry review.
Mole  Atomic and Molecular Weights
Categories of Chemical Reactions
Oxidation Numbers, Redox Reactions, Oxidizing vs. Reducing Agents
Mixtures
Follow the direction of successive arrows moving from top to bottom
The order for filling atomic orbitals
Metals, Nonmetals and Metalloids
*General Characteristics of metals, nonmetals and metalloids
This polar bond will also have a dipole moment given by:
The Lewis acid BF_{3} and the Lewis base NH_{3}. Notice that the green arrows follow the flow of electron pairs.
Geometry of simple molecules in which the central atom A has one or more lone pairs of electrons (= e^{})
Note: dotted lines only represent the overall molecular shape and not molecular bonds. In brackets under "Molecular Geometry" is the hybridization as discussed in ORG 1.2.
The Maxwell Distribution Plot
Graham’s Law (Diffusion and Effusion of Gases)

Combined Gas Law

Charles’ Law

Ideal Gas Law
since m/V is the density (d) of the gas: 
Boyle’s Law

Partial Pressure and Dalton’s Law
ΣX_{1} = 1 
Avogadro’s Law

The partial pressure (P_{i}) of a component of a gas mixture is equal to:

Liquid Phase (Intra and Intermolecular Forces)
Van Der Waal's forces (weak) and hydrogen bonding (strong). London forces between Cl_{2} molecules, dipoledipole forces between HCl molecules and Hbonding between H_{2}O molecules. Note that a partial negative charge on an atom is indicated by ẟ (delta negative), while a partial positive charge is indicated by ẟ+ (delta positive). Notice that one H_{2}O molecule can potentially form 4 Hbonds with surrounding molecules which is highly efficient. The preceding is one key reason that the boiling point of water is higher than that of ammonia, hydrogen fluoride, or methanol.
Phase diagram of water demonstrating the effect of the addition of a solute
Common Anions and Cations
Because the K_{sp} product always holds, precipitation will not take place unless the product of [Ag^{+}] and [Cl^{}] exceeds the K_{sp}.
Acids
STRONG  WEAK 

Perchloric HClO_{4} Chloric HClO_{3} Nitric HNO_{3} Hydrochloric HCl Sulfuric H_{2}SO_{4} Hydrobromic HBr Hydriodic HI Hydronium Ion H_{3}O^{+} 
Hydrocyanic HCN Hypochlorous HClO Nitrous HNO_{2} Hydrofluoric HF Sulfurous H_{2}SO_{3} Hydrogen Sulfide H_{2}S Phosphoric H_{3}PO_{4} Benzoic, Acetic and other Carboxylic Acids 
Water Dissociation
Salts of Weak Acids and Bases
Buffers
Bases
at 25°C, pH + pOH = 14.0
The First Law of Thermodynamics
Temperature Scales
State Functions
W can be determined experimentally by calculating the area under a pressurevolume curve
Work  Heat  Changes in internal energy  

1st tranf.  w  0  w 
2nd transf.  W = w +q  q  w 
If a reaction requires the supply of a certain amount of heat it is endothermic (ΔH is positive).
Bond Dissociation Energies and Heats of Formation
Calorimetry
The Second Law of Thermodynamics
Entropy
Free Energy
Dependence of Reaction Rates on Concentration of Reactants
Dependence of Reaction Rates upon Temperature
Potential Energy Diagrams: Exothermic vs. Endothermic Reactions
Catalysis
Potential Energy Diagrams: Without and With a Catalyst
Saturation Kinetics
Equilibrium in Reversible Chemical Reactions
{Note: Catalysts speed up the rate of reaction without affecting K_{eq}}
Le Chatelier’s Principle
Relationship between the Equilibrium Constant and the Change in the Gibbs Free Energy
Generalities
Galvanic Cells
Concentration Cell
Faraday’s Law
Glassware
Least accurate  Droppers Beakers Erlenmeyer flasks Graduated cylinders 
Most accurate  Glass Pipettes
Burettes Volumetric flasks 
Analyzing the Data
Significant  Examples  NonSignificant 

Nonzero integers  1.234 (4 sf)  
Zeros between nonzero integers*  1.004 (4 sf)  
Zeros to the right of decimal place AND integers*  1.2000 (5 sf) 0.0041 (2 sf) 
Zeros to the right of decimal place BUT to the left of integers 
430 (2 sf)  Zeros to the left of decimal place BUT to the right of integers  
013.2 (2 sf)  Zeros to the left of decimal place AND integers 
*Zeros in any number are used to convey either accuracy or magnitude. If a zero is to convey accuracy, then it is known as a significant value and if the zero is used to convey magnitude, then it is nonsignificant.
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